Unit four JCL

Question 1

Group 1 metals oxidation state

Answer 1

always +1

Question 2

Group 2 metals oxidation state

Answer 2

always +2

Question 3

Oxygen oxidation state

Answer 3

usually -2 (except in peroxides, where it is -1 and F2O, where it is +2)

Question 4

Hydrogen oxidation state

Answer 4

usually +1 (except in metal hydrides, where it is -1)

Question 5

Fluorine oxidation state

Answer 5

always -1

Question 6

Chlorine oxidation state

Answer 6

usually -1 (except in compounds with O or F)

Question 7

What increases as you go down group 2

Answer 7

Reactivity, Atomic Radius, Reaction with water, Solubility of Hydroxide

Question 8

What decreases as you go down group 2

Answer 8

1st ionization energy, Melting point, Solubility of Sulfate

Question 9

What are oxidizing agents

Answer 9

They cause anther species to be oxidized by taking electrons, The oxidizing agents themselves are reduced

Question 10

What is a displacement reaction

Answer 10

A reaction in which a more reactive element displaces a less reactive element from an aqueous solution of its ion

Question 11

What colour is the water and cyclohexane for Cl2

Answer 11

water: pale-green
cyclohexane: pale-green

Question 12

What colour is the water and cyclohexane for Br2

Answer 12

water: Orange
cyclohexane: Orange

Question 13

What colour is the water and cyclohexane for I2

Answer 13

water: Brown
cyclohexane: Violet

Question 14

What is a disproportionation reaction

Answer 14

A redox reaction in which the same element is both oxidised and reduced

Question 15

Identifying halide ions, precipitate colour

Answer 15

AgCl: white
AgBr: cream
AgI: yellow

Question 16

Identifying halide ions, solubility of silver halide solution in NH3

Answer 16

AgCl: soluble in dilute NH3 (ammonia)
AgBr: soluble in concentrated NH3
AgI: insoluble in concentrated NH3

Question 17

What is the trend in oxidising power down group seven?

Answer 17

It decreases

Question 18

Test for carbonate ion?

Answer 18

Put in dilute acid, bubble through lime water, turns cloudy

Question 19

Test for sulphate ion?

Answer 19

Add barium chloride, forms white precipitate

Question 20

Test for ammonium ion?

Answer 20

Add sodium hydroxide and heat, red litmus paper will turn blue from ammonia gas produced

Question 21

Define first ionization energy

Answer 21

The first ionization energy of an element is the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions

Question 22

Define successive ionisation energy

Answer 22

Successive ionization energies of an element are a measure of the energy required to remove each electron in turn

Question 23

How does electron shielding effect ionization energy?

Answer 23

More inner shell electrons –> greater distance –> less nuclear attraction on outer shell electrons

Question 24

How does atomic radius effect ionization energy?

Answer 24

Greater radius –> less nuclear attraction on outer shell electrons

Question 25

How does nuclear charge effect ionization energy?

Answer 25

Greater nuclear charge --> greater attractive force on the outer shell electrons

Question 26

Why is there a drop in first ionization energy between p and s?

Answer 26

The electrons are in a new sub-shell that is higher in energy so it takes less energy to remove an electron

Question 27

Why is sodium described as an s-block element?

Answer 27

Its outermost electron is in the s sub-shell

Question 28

What is metallic bonding?

Answer 28

The electrostatic attraction between po0sitive metal ions and delocalized electrons

Question 29

What does delocalized mean?

Answer 29

Electrons are free to move and are not fixed to one specific ion/atom

Question 30

What does the word lattice mean?

Answer 30

A regularly repeating pattern

Question 31

What is a giant metallic lattice?

Answer 31

A 3D structure of regularly arranged positive ions in a sea of delocalized electrons bonded by strong metallic bonds

Question 32

Melting/ boiling point in metals

Answer 32

High melting and boiling points

Question 33

Electrical conductivity in metals

Answer 33

Good conductivity

Question 34

Physical manoeuvability

Answer 34

Malleable and ductile

Question 35

Malleable definition

Answer 35

Can be hammered into shape

Question 36

Ductile definition

Answer 36

Can be drawn out into wires

Question 37

Why do metals have high melting and boiling points

Answer 37

Strong electrostatic attraction between positive metal ions and negative electrons, metallic bonds require high amounts of energy to break apart

Question 38

Why are metals good conducters

Answer 38

Delocalized electrons are free to move across the metallic lattice and can carry a charge in a uniform direction producing a current

Question 39

Why are metals malleable and ductile?

Answer 39

Delocalized electrons can move and layers in the giant metallic lattice are able to slide over each over